21 SO2Recovery by a sodium citrate solution scrubbing

Erga, Olav

doi:10.1016/0009-2509(80)80083-2

Cited by 20 publications

(11 citation statements)

References 3 publications

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“…Like other regeneration methods, there are some advantages when CaL 2 method is used for the capture of SO 2 , such as regeneration of absorbent, recovery of SO 2 and reduction of by-product. In other regeneration processes, for example sodium method [3,4] and ionic liquid method [22,23], both the absorbent (Na 2 SO 3 , Na 3 C 6 H 5 O 7 and IL) and by-product (Na 2 SO 4 and IL-SO 4 ) are water-soluble. As a result, it is very difficult to separate the by-product from the absorbent.…”

Section: Comparison Of Cal 2 Methods With Other Methodsmentioning

confidence: 99%

“…Therefore, regenerable technologies show many advantages for the capture of SO 2 . It is well known that sodium method [3,4], magnesium method [5,6] and amine method [7,8] have been commercially used in the process of desulfurization of flue gas. Besides the commercially used methods, the absorption of SO 2 by recyclable organic solvents [9,10] or ionic liquids (ILs) [11][12][13][14][15] has also been proposed by researchers in recent years.…”

Section: Introductionmentioning

confidence: 99%

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Reversible absorption of SO2 from simulated flue gas by aqueous calcium lactate solution

Tian

Hou

et al. 2015

Journal of the Taiwan Institute of Chemical Engineers

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Section: Comparison Of Cal 2 Methods With Other Methodsmentioning

confidence: 99%

Section: Introductionmentioning

confidence: 99%

Reversible absorption of SO2 from simulated flue gas by aqueous calcium lactate solution

Tian

Hou

et al. 2015

Journal of the Taiwan Institute of Chemical Engineers

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“…Citrate salts, which are derived from a natural product, citric acid, are used to form buffer solutions that can be used for SO 2 scrubbing. 8,9 However, issues have been observed upon process scale-up including fouling of piping and equipment, as well as SO 2 oxidation to SO 3 , which will form H 2 SO 4 in the presence of water.…”

Section: Introductionmentioning

confidence: 99%

Chemical and Physical Absorption of SO₂ by N-Functionalized Imidazoles: Experimental Results and Molecular-level Insight

Shannon

Irvin

Liu

et al. 2014

Ind. Eng. Chem. Res.

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Sulfur dioxide (SO 2 ) removal is a key component of many industrial processes, especially coal-fired power generation. Controlling SO 2 emissions is vital to maintaining environmental quality, as SO 2 is a contributor to acid rain, but has value as a chemical feedstock. Although a number of novel solvents/materials including ionic liquids (ILs) have recently been proposed for alternatives to limestone scrubbing for SO 2 capture/removal from point sources, the imidazole architecture presents a convenient, inexpensive and efficient class of low volatility and low viscosity solvents to accomplish this goal. On the basis of our prior work with imidazoles for CO 2 capture, we have extended our interests toward understanding the relationship between imidazole structure and SO 2 absorption. Using a series of imidazole compounds with various substituents at the 1, 2 and/or 4(5) positions of the five-membered ring, SO 2 absorption via both chemical and physical mechanisms was observed. The chemical absorption product is a relatively stable 1:1 SO 2 −imidazole complex, while physical absorption of SO 2 is dependent on pressure and temperature. Because imidazoles are relatively small molecules, they are an efficient absorption medium for SO 2 and can form adducts wherein the mass fraction of bound SO 2 is >40 wt %. The SO 2 −imidazole complexes were also observed to produce distinct color and/or phase changes that are associated with the nature of the substituents present. The chemically bound SO 2 can be released under vacuum at moderate temperature (∼100°C) and vacuum, yielding the original neat solvent, while the physically dissolved SO 2 can be readily removed at ambient temperature under vacuum. This behavior corresponds to a much smaller enthalpy of absorption for physical dissolution (−4 to −13 kJ/mol) as determined via thermodynamic relationships compared to the binding energies of chemical complexation (−35 to −42 kJ/mol) as determined via density functional theory calculations. Increasing chemical complexation energies are correlated with increased substitution on the imidazole ring. Simulations were also employed to gain insight into the structures of the SO 2 −imidazole complexes, illustrating changes in partial charge distribution before and after complexation as well as confirming a charge transfer complex is formed based on the N−S bond length.

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“…This finding follows from an analysis of the measured pH and gasliquid equilibrium data, in much the same way as achieved earlier for citrate and adipate buffered SO, solutions [7,81.…”

Section: Comparison With Experimental Equilibrium Datamentioning

confidence: 86%

Equilibrium model for CO₂ absorption in an aqueous solution of 2‐amino‐2‐methyl‐1‐propanol

Erga

Lidal

1991

Chem Eng & Technol

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A semi-empirical gas-liquid equilibrium model for the absorption of CO, in aqueous 3M AMP (2-amino-2-methyl-I-propanol) is presented. It applies to high CO, loadings (y > 0.5) in the temperature range between 20 and 50 "C, and is based on experimental solubility and pH determinations. For a given amine concentration, it yields the equilibrium partial pressure of CO, as a function of only two variables: the CO, loading and temperature. The model correlates the expressions for the chemical equilibria involved as follows: pco, = m y x lo", where pco, is the equilibrium partial pressure, x = logK -pH, m is the amine molarity, y the CO, loading, and K is a parameter involving Henry's law constant, H, and the first dissociation constant, K,, of carbonic acid. pH is found to depend on both temperature and CO, loading while logK depends only on the CO, loading. Correlations for pH and logK are presented. The model fits own data for 3M AMP very well as well as the equilibrium data found in recent literature.

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21 SO2Recovery by a sodium citrate solution scrubbing

Cited by 20 publications

References 3 publications

Reversible absorption of SO2 from simulated flue gas by aqueous calcium lactate solution

Reversible absorption of SO2 from simulated flue gas by aqueous calcium lactate solution

Chemical and Physical Absorption of SO₂ by N-Functionalized Imidazoles: Experimental Results and Molecular-level Insight

Equilibrium model for CO₂ absorption in an aqueous solution of 2‐amino‐2‐methyl‐1‐propanol

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21 SO2Recovery by a sodium citrate solution scrubbing

Cited by 20 publications

References 3 publications

Reversible absorption of SO2 from simulated flue gas by aqueous calcium lactate solution

Reversible absorption of SO2 from simulated flue gas by aqueous calcium lactate solution

Chemical and Physical Absorption of SO2 by N-Functionalized Imidazoles: Experimental Results and Molecular-level Insight

Equilibrium model for CO2 absorption in an aqueous solution of 2‐amino‐2‐methyl‐1‐propanol

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Chemical and Physical Absorption of SO₂ by N-Functionalized Imidazoles: Experimental Results and Molecular-level Insight

Equilibrium model for CO₂ absorption in an aqueous solution of 2‐amino‐2‐methyl‐1‐propanol